Bonding
No description yet. This curated deck is ready for daily study.
Card preview (12)
Define electronegativity [1]
[1] Atom’s ability to attract the lone pair of electrons
Why is the C-Cl bond polar? [2]
[1] Cl is highly electronegative [2] so the electron density is not symmetrical
Why is CCl4 non polar? [2]
[1] It is a symmetrical molecule [2] So dipoles cancel out
Whatcauses VdW forces between non polar molecules? [3]
[1] Random movement of electrons [2] Induces a dipole in another molecule [3] Dipoles in different molecules attract
In terms of intermolecular forces, why does CBr4 have a higher boiling point than CHBr3 [3]
[1] CBr4 have VdW forces [2] CHBr3 have VdW forces and permanent dipole-dipole forces [3] CBr4 have stronger intermolecular forces
Ionic bonding properties
Electrostatic attraction between two oppositely charged ions. Soluble as polar. Conducts electricty when molten or dissolved in solution as ions are free to move. High m.p
Simple molecular covalent properties
Electrostatic attraction between sharing of outer electrons in NM. Lower b.p as weak intermolecular forces. Solubility dependant on polarity. Cannot conduct electricity. Brittle due to weak intermolecular forces.
Properties of graphite
Carbon bonded 3 times with 4th electron delocalised. Can carry charge. Layers slide over eachother easily due to weak inbetween forces. High b.p Low density layers Insoluble
Graphene properties
Can conduct electricity. Insoluble. 2D so less resistance. High mp and bp
Diamond properties
Carbon bonded 4 times. Cannot conduct electricity due to no delocalised electrons. Can conduct heat well. Insoluble. High bp
Metallic properties
Electrostatic attraction between metal ions and delocalised electron. More positive the metal = higher the bp Good thermal and electrical conducters. Insoluble
Ice properties
Polar bond with strong H bonds Water into ice becomes less dense as H bonding pushed molecules futher apart